You have two containers of equal volume. one is full of helium gas. the other holds an equal mass of nitrogen gas both gases hav

Assuming both He and N₂ behave as ideal gases, we apply the ideal gas law, PV = nRT, where P represents gas pressure, V is volume, n refers to the number of moles, R is the universal gas constant, and T indicates temperature in Kelvin. For both gases, P and V are identical. R remains a constant. The variations only involve n and T. Let’s define the temperature of He as T₁ and that of N₂ as T₂. The moles are calculated as n = m/M, where n signifies moles, m is mass, and M stands for molar mass. The molar mass of He is 4 g/mol while for N₂ it is 28 g/mol. Since the mass of both gases remains constant, the moles of He = m/4 and the moles of N₂ = m/28. Applying the ideal gas equation for both gases, for He, we have PV = (m/4)RT₁ and for N₂, PV = (m/28)RT₂. Equating both results leads to T₁/4 = T₂/28, implying T₁ = T₂/7. Thus, the temperature of nitrogen gas is 7 times greater than that of helium.